MnO^{-}_4 is of intense pink colour,though Mn | vedclass

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(C) The intense color in $MnO^{-}_4$ arises from a ligand-to-metal charge transfer $(LMCT)$ transition.In $MnO^{-}_4$,$Mn$ is in the $(+7)$ oxidation

Vedclass · Accepted Answer

Charge transfer when oxygen gives its electron to $Mn(+7)$ changing in $Mn(+6)$

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(C) The intense color in $MnO^{-}_4$ arises from a ligand-to-metal charge transfer $(LMCT)$ transition.In $MnO^{-}_4$,$Mn$ is in the $(+7)$ oxidation state,meaning it has a $d^0$ electronic configuration.Since there are no $d$-electrons,a $d-d$ transition is impossible.The color arises because an electron is transferred from the oxygen $2p$ orbitals to the empty $3d$ orbitals of the $Mn(+7)$ ion upon the absorption of light.This electronic transition corresponds to the energy of yellow light,which is absorbed,resulting in the observation of the complementary color,which is intense pink or purple.

$MnO^{-}_4$ is of intense pink colour,though $Mn$ is in $(+7)$ oxidation state,it is due to

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